Chapter 4: Aromatic Compounds. Bitter almonds are the source of the aromatic compound benzaldehyde

Transcription

1 Chapter 4: Aromatic Compounds Bitter almonds are the source of the aromatic compound benzaldehyde

2 Sources of Benzene Benzene, C 6 H 6, is the parent hydrocarbon of the especially stable compounds known as aromatic compounds.

3 4.1 Some Facts About Benzene -The carbon-to-hydrogen ratio in benzene, C 6 H 6,suggests a highly unsaturated structure. -Despite its molecular formula, benzene for the most part does not behave as if it were unsaturated. - it does not decolorize bromine solutions. -it not easily oxidized by potassium permanganate. Reacts mainly by substitution

4 4.2 The Kekulé Structure for Benzene In 1865, Kekulé proposed a reasonable structure for benzene Kekulé s two structures for benzene differ only in the arrangement of the electrons; all of the atoms occupy the same positions in both structures.

5 4.3 The Resonance Structure of Benzene Modern physical measurements support this model for the benzene structure: - Benzene is planar. - Each carbon atom is at the corner of a regular hexagon. - All of the carbon carbon bond lengths are identical: 1.39 Å, intermediate between typical single (1.54 Å) and double (1.34 Å) carbon carbon bond lengths.

6 4.4 The Orbital Model for Benzene The p orbitals on all six carbon atoms can overlap laterally to form pi orbitals that create a ring or cloud of electrons above and below the plane of the ring. 4.5 Symbols for Benzene

7 4.6 Nomenclature of Aromatic Compounds Common names have acquired historic respectability and are accepted by IUPAC. Monosubstituted benzenes with common names

8 Monosubstituted benzenes that do not have common names When two substituents are present, we use prefixes ortho-, meta-, and para-, usually abbreviated as o-, m-, and p-, respectively.

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10 For more than two substituents, their positions are designated by numbering the ring.

11 Aromatic hydrocarbons, as a class called Arenes (Ar) the aryl groups are therefore aromatic substituents.

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14 4.7 The Resonance Energy of Benzene Hydrogenation of a carbon carbon double bond is an exothermic reaction. The amount of energy (heat) released is about 26 to 30 kcal/mol. for each double bond. Hydrogenation of cyclohexene releases 28.6 kcal/mol. The complete hydrogenation of 1,3-cyclohexadiene should release twice that amount of heat, or 2 X 28.6 = 57.2 kcal/mol.

15 The hypothetical triene 1,3,5-cyclohexatriene should correspond to that for three double bonds, or about 84 to 86 kcal/mol. That benzene is more difficult to hydrogenate than simple alkenes, and the heat evolved when benzene is hydrogenated to cyclohexane is much lower than expected: only 49.8 kcal/mol.

16 We conclude that real benzene molecules are more stable than the contributing resonance structures (the hypothetical molecule 1,3,5- cyclohexatriene) by about 36 kcal/mol (86-50 = 36). The stabilization energy, or resonance energy, of a substance is the difference between the energy of the real molecule and the calculated energy of the most stable contributing structure. Benzene and other aromatic compounds usually react in such a way as to preserve their aromatic structure and therefore retain their resonance energy.

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18 4.8 Electrophilic Aromatic Substitution The most common reactions of aromatic compounds involve substitution of other atoms or groups for a ring hydrogen on the aromatic unit.

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20 4.9 The Mechanisms of Electrophilic Substitutions For Example, Chlorination of Benzene Ferric chloride acts as a Lewis acid and converts chlorine to a strong electrophile by forming a complex and polarizing the Cl-Cl bond.

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23 b. Nitration

24 c. sulfonation

25 d. Alkylation and Acylation (Friedel-Crafts reaction)

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27 4.10 Ring-Activating and ring-deactivating Substituents Consider the relative nitration rates of the following compounds, all under the same reaction conditions:

28 In the electrophilic mechanism for substitution: Substituents that donate electrons to the ring will increase its electron density and, hence, speed up the reaction. Substituents that withdraw electrons from the ring will decrease electron density in the ring and therefore slow down the reaction.

29 4.11 Ortho, Para-Directing and Meta-Directing Groups Substituents already present on an aromatic ring determine the position taken by a new substituent.

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31 a. Ortho, Para-Directing Groups

32 Consider now the other ortho,para-directing groups. In each of them, the atom attached to the aromatic ring has an unshared electron pair. This unshared electron pair can stabilize an adjacent positive charge.

33 Let us consider, as an example, the bromination of phenol.

34 In the case of o- or p- attack, one of the contributors to the intermediate benzenonium ion places the positive charge on the hydroxyl-bearing carbon. Shift of an unshared electron pair from the oxygen to the positive carbon allows the positive charge to be delocalized even further, onto the oxygen.

35 b. meta-directing Groups

36 One of the contributors to the resonance hybrid intermediate for ortho or para substitution (shown in the blue dashed boxes) has two adjacent positive charges, a highly undesirable arrangement, because like charges repel each other. No such intermediate is present for meta substitution. For this reason, meta substitution is preferred.

37 All groups in which the atom directly attached to the aromatic ring is positively charged or is part of a multiple bond to a more electronegative element will be meta directing.

38 c. Substituent Effect on Reactivity In all meta-directing groups, the atom connected to the ring carries a full or partial positive charge and will therefore withdraw electrons from the ring. All meta-directing groups are therefore ringdeactivating groups. On the other hand, ortho,para-directing groups in general supply electrons to the ring and are therefore ring activating. With the halogens (F, Cl, Br, and I), two opposing effects bring about the only important exception to these rules. Because they are strongly electron withdrawing, the halogens are ring deactivating; but because they have unshared electron pairs, they are ortho,para-directing.

39 4.12 Importance of Directing Effects in Synthesis

40 PROBLEM 4.16 Devise a synthesis for each of the following, starting with benzene: a. m-bromobenzenesulfonic acid b. p-nitrotoluene

41 Homework